Consider a solution containing liquids A and B where the mole fraction of B is 0.60.Assuming ideality,calculate the mole fraction of B in the vapor at equilibrium with this solution at 25°C.(The vapor pressures of pure liquid A and B at 25°C are 129.4 torr and 400.0 torr,respectively. )
A)0.18
B)0.22
C)0.33
D)0.78
E)0.82

Question

Quizplus · Accepted Answer

The mole fraction of B in the vapor phase can be calculated using Raoult's Law and Dalton's Law. The partial pressure of B is 0.60 * 400.0 torr = 240.0 torr, and for A, it is 0.40 * 129.4 torr = 51.76 torr. The total pressure is 240.0 + 51.76 = 291.76 torr. The mole fraction of B in the vapor is 240.0 / 291.76 ≈ 0.82.

Consider a Solution Containing Liquids a and B Where the Mole